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Suppose 1.00 mol water at 25°C is flash-evaporated by allowing it to fall into an iron crucible maintained at 150°C. Calculate ΔS for the water, ΔS for the iron crucible.



Answer :

The enthalpy of vaporization of water (ΔS) is 40.68 kJ [tex]mol^{-1}[/tex].

Number of moles of water (n) = 1.00 mol

Temperature of water, (T) = 25°C

Convert into kelvin,

The temperature of water,(T)  = 25 + 273.15

                                          = 298.15K

Heat capacity of liquid water,

[tex]C_{p}[/tex][H20(l)]=  75.4 L [tex]K^{-1}[/tex] [tex]mol^{-1}[/tex]

Heat capacity of liquid water,

[tex]c_{p}[/tex][H20(g)] = 36.0 J[tex]K^{-1}[/tex] [tex]mol^{-1}[/tex]

Enthalpy of vaporization of water,

ΔS = 40.68 KJ[tex]mol^{-1}[/tex]

To know about the enthalpy of vaporization refer to the link given below:

https://brainly.com/question/13776849

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